Nitrogen dioxide

Last updated
Nitrogen dioxide
Skeletal formula of nitrogen dioxide with some measurementsEP Nitrogen-dioxide-2D-dimensions-vector.svg
Skeletal formula of nitrogen dioxide with some measurementsEP
Spacefill model of nitrogen dioxide Nitrogen-dioxide-3D-vdW.png
Spacefill model of nitrogen dioxide
Nitrogen dioxide at different temperatures.jpg
NO
2 converts to the colorless dinitrogen tetroxide (N
2O
4) at low temperatures and reverts to NO
2 at higher temperatures.
Names
IUPAC name
Nitrogen dioxide
Other names
Nitrogen(IV) oxide, [1] deutoxide of nitrogen
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.030.234 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 233-272-6
976
PubChem CID
RTECS number
  • QW9800000
UNII
UN number 1067
  • InChI=1S/NO2/c2-1-3 Yes check.svgY
    Key: JCXJVPUVTGWSNB-UHFFFAOYSA-N Yes check.svgY
  • InChI=1/NO2/c2-1-3
    Key: JCXJVPUVTGWSNB-UHFFFAOYAA
  • N(=O)[O]
  • [N+](=O)[O-]
Properties
NO•
2
Molar mass 46.005 g·mol−1
AppearanceBrown gas [2]
Odor Chlorine-like
Density 1.880 g/L [2]
Melting point −9.3 °C (15.3 °F; 263.8 K) [2]
Boiling point 21.15 °C (70.07 °F; 294.30 K) [2]
Hydrolyses
Solubility Soluble in CCl
4, nitric acid, [3] chloroform
Vapor pressure 98.80 kPa (at 20 °C)
+150.0·10−6 cm3/mol [4]
1.449 (at 20 °C)
Structure
C2v
Bent
Thermochemistry [5]
37.2 J/(mol·K)
Std molar
entropy (S⦵298)
240.1 J/(mol·K)
+33.2 kJ/mol
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
Poison, oxidizer
GHS labelling:
GHS-pictogram-rondflam.svg GHS-pictogram-bottle.svg GHS-pictogram-acid.svg GHS-pictogram-skull.svg GHS-pictogram-silhouette.svg
Danger
H270, H314, H330
P220, P260, P280, P284, P305+P351+P338, P310
NFPA 704 (fire diamond)
NFPA 704.svgHealth 4: Very short exposure could cause death or major residual injury. E.g. VX gasFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
4
0
0
OX
Lethal dose or concentration (LD, LC):
30 ppm (guinea pig, 1  h)
315 ppm (rabbit, 15 min)
68 ppm (rat, 4 h)
138 ppm (rat, 30 min)
1000 ppm (mouse, 10 min) [6]
64 ppm (dog, 8 h)
64 ppm (monkey, 8 h) [6]
NIOSH (US health exposure limits):
PEL (Permissible)
C 5 ppm (9 mg/m3) [7]
REL (Recommended)
ST 1 ppm (1.8 mg/m3) [7]
IDLH (Immediate danger)
13 ppm [7]
Safety data sheet (SDS) ICSC 0930
Related compounds
Dinitrogen pentoxide

Dinitrogen tetroxide
Dinitrogen trioxide
Nitric oxide
Nitrous oxide

Contents

Related compounds
 Chlorine dioxide
Carbon dioxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)

Nitrogen dioxide is a chemical compound with the formula NO2. One of several nitrogen oxides, nitrogen dioxide is a reddish-brown gas. It is a paramagnetic, bent molecule with C2v point group symmetry. Industrially, NO2 is an intermediate in the synthesis of nitric acid, millions of tons of which are produced each year, primarily for the production of fertilizers.

Nitrogen dioxide is poisonous and can be fatal if inhaled in large quantities. [8] The LC50 (median lethal dose) for humans has been estimated to be 174 ppm for a 1-hour exposure. [9] It is also included in the NOx family of atmospheric pollutants.

Properties

Nitrogen dioxide is a reddish-brown gas with a pungent, acrid odor above 21.2 °C (70.2 °F; 294.3 K) and becomes a yellowish-brown liquid below 21.2 °C (70.2 °F; 294.3 K). It forms an equilibrium with its dimer, dinitrogen tetroxide (N2O4), and converts almost entirely to N2O4 below −11.2 °C (11.8 °F; 261.9 K). [7]

The bond length between the nitrogen atom and the oxygen atom is 119.7  pm. This bond length is consistent with a bond order between one and two.

Unlike ozone (O3) the ground electronic state of nitrogen dioxide is a doublet state, since nitrogen has one unpaired electron, [10] which decreases the alpha effect compared with nitrite and creates a weak bonding interaction with the oxygen lone pairs. The lone electron in NO2 also means that this compound is a free radical, so the formula for nitrogen dioxide is often written as •NO2.

The reddish-brown color is a consequence of preferential absorption of light in the blue region of the spectrum (400–500 nm), although the absorption extends throughout the visible (at shorter wavelengths) and into the infrared (at longer wavelengths). Absorption of light at wavelengths shorter than about 400 nm results in photolysis (to form NO + O, atomic oxygen); in the atmosphere the addition of the oxygen atom so formed to O2 results in ozone.

Preparation

Nitrogen dioxide typically arises via the oxidation of nitric oxide by oxygen in air (e.g. as result of corona discharge): [11]

2 NO + O2 → 2 NO2

Nitrogen dioxide is formed in most combustion processes using air as the oxidant. At elevated temperatures nitrogen combines with oxygen to form nitrogen dioxide:

 N2 + 2 O2 → 2 NO2

In the laboratory, NO
2 can be prepared in a two-step procedure where dehydration of nitric acid produces dinitrogen pentoxide:

2 HNO3 → N2O5 + H2O
6 HNO3 +1⁄2 P4O10 → 3 N2O5 + 2 H3PO4

which subsequently undergoes thermal decomposition:

N2O5 → 2 NO2 +1⁄2 O2

The thermal decomposition of some metal nitrates also generates NO2:

Pb(NO3)2 → PbO + 2 NO2 +1⁄2 O2

NO2 is generated by the reduction of concentrated nitric acid with a metal (such as copper):

4 HNO3 + Cu → Cu(NO3)2 + 2 NO2 + 2 H2O

Formation from decomposition of nitric acid

Nitric acid decomposes slowly to nitrogen dioxide by the overall reaction:

4 HNO3 → 4 NO2 + 2 H2O + O2

The nitrogen dioxide so formed confers the characteristic yellow color often exhibited by this acid.

Selected reactions

Thermal properties

NO2 exists in equilibrium with the colourless gas dinitrogen tetroxide (N2O4):

2 NO2 ⇌ N2O4

The equilibrium is characterized by ΔH = −57.23 kJ/mol, which is exothermic. NO2 is favored at higher temperatures, while at lower temperatures, N2O4 predominates. N2O4 can be obtained as a white solid with melting point −11.2 °C. [11] NO2 is paramagnetic due to its unpaired electron, while N2O4 is diamagnetic.

At 150 °C (302 °F; 423 K), NO2 decomposes with release of oxygen via an endothermic process (ΔH = 14 kJ/mol):

2 NO2 →2 NO +  O2

As an oxidizer

As suggested by the weakness of the N–O bond, NO2 is a good oxidizer. Consequently, it will combust, sometimes explosively, in the presence of hydrocarbons. [12]

Hydrolysis

NO2 reacts with water to give nitric acid and nitrous acid:

3 NO2 + H2O → HNO3 + HNO2

This reaction is one of the steps in the Ostwald process for the industrial production of nitric acid from ammonia. [13] This reaction is negligibly slow at low concentrations of NO2 characteristic of the ambient atmosphere, although it does proceed upon NO2 uptake to surfaces. Such surface reaction is thought to produce gaseous HNO2 (often written as HONO) in outdoor and indoor environments. [14]

Conversion to nitrates

NO2 is used to generate anhydrous metal nitrates from the oxides: [11]

MO + 3 NO2 → M(NO3)2 + NO

Alkyl and metal iodides give the corresponding nitrates: [10]

TiI4 + 8 NO2 → Ti(NO3)4 + 4 NO + 2 I2

Ecology

NO2 is introduced into the environment by natural causes, including entry from the stratosphere, bacterial respiration, volcanos, and lightning. These sources make NO2 a trace gas in the atmosphere of Earth, where it plays a role in absorbing sunlight and regulating the chemistry of the troposphere, especially in determining ozone concentrations. [15]

Uses

NO2 is used as an intermediate in the manufacturing of nitric acid, as a nitrating agent in the manufacturing of chemical explosives, as a polymerization inhibitor for acrylates, as a flour bleaching agent, [16] : 223  and as a room temperature sterilization agent. [17] It is also used as an oxidizer in rocket fuel, for example in red fuming nitric acid; it was used in the Titan rockets, to launch Project Gemini, in the maneuvering thrusters of the Space Shuttle, and in uncrewed space probes sent to various planets. [18]

Human-caused sources and exposure

A "fox tail" over Nizhniy Tagil Iron and Steel Works Nizhniy tagil ntmk main entrance.JPG
A "fox tail" over Nizhniy Tagil Iron and Steel Works

For the general public, the most prominent sources of NO2 are internal combustion engines, as combustion temperatures are high enough to thermally combine some of the nitrogen and oxygen in the air to form NO2. [8] Outdoors, NO2 can be a result of traffic from motor vehicles. [19]

Indoors, exposure arises from cigarette smoke, [20] and butane and kerosene heaters and stoves. [21]

Workers in industries where NO2 is used are also exposed and are at risk for occupational lung diseases, and NIOSH has set exposure limits and safety standards. [7] Workers in high voltage areas especially those with spark or plasma creation are at risk.[ citation needed ] Agricultural workers can be exposed to NO2 arising from grain decomposing in silos; chronic exposure can lead to lung damage in a condition called "silo-filler's disease". [22] [23]

Toxicity

NO2 diffuses into the epithelial lining fluid (ELF) of the respiratory epithelium and dissolves. There, it chemically reacts with antioxidant and lipid molecules in the ELF. The health effects of NO2 are caused by the reaction products or their metabolites, which are reactive nitrogen species and reactive oxygen species that can drive bronchoconstriction, inflammation, reduced immune response, and may have effects on the heart. [24]

Pathways indicated by a dotted line are those for which evidence is limited to findings from experimental animal studies, while evidence from controlled human exposure studies is available for pathways indicated by a solid line. Dashed lines indicate proposed links to the outcomes of asthma exacerbation and respiratory tract infections. Key events are subclinical effects, endpoints are effects that are generally measured in the clinic, and outcomes are health effects at the organism level. NO2 = nitrogen dioxide; ELF = epithelial lining fluid. No2toxpathwaysEPA.png
Pathways indicated by a dotted line are those for which evidence is limited to findings from experimental animal studies, while evidence from controlled human exposure studies is available for pathways indicated by a solid line. Dashed lines indicate proposed links to the outcomes of asthma exacerbation and respiratory tract infections. Key events are subclinical effects, endpoints are effects that are generally measured in the clinic, and outcomes are health effects at the organism level. NO2 = nitrogen dioxide; ELF = epithelial lining fluid.
Nitrogen dioxide diffusion tube for air quality monitoring. Positioned in the City of London. AirQualityLondon1.jpg
Nitrogen dioxide diffusion tube for air quality monitoring. Positioned in the City of London.

Acute harm due to NO2 exposure is rare. 100–200 ppm can cause mild irritation of the nose and throat, 250–500 ppm can cause edema, leading to bronchitis or pneumonia, and levels above 1000 ppm can cause death due to asphyxiation from fluid in the lungs. There are often no symptoms at the time of exposure other than transient cough, fatigue or nausea, but over hours inflammation in the lungs causes edema. [25] [26]

For skin or eye exposure, the affected area is flushed with saline. For inhalation, oxygen is administered, bronchodilators may be administered, and if there are signs of methemoglobinemia, a condition that arises when nitrogen-based compounds affect the hemoglobin in red blood cells, methylene blue may be administered. [27] [28]

It is classified as an extremely hazardous substance in the United States as defined in Section 302 of the U.S. Emergency Planning and Community Right-to-Know Act (42 U.S.C. 11002), and it is subject to strict reporting requirements by facilities which produce, store, or use it in significant quantities. [29]

Health effects of NO2 exposure

Exposure to low levels of NO2 over time can cause changes in lung function. [30] Chronic exposure to NO2 can cause respiratory effects including airway inflammation in healthy people and increased respiratory symptoms in people with asthma.

The effects of toxicity on health have been examined using questionnaires and in-person interviews in an effort to understand the relationship between NO2 and asthma. The influence of indoor air pollutants on health is important because the majority of people in the world spend more than 80% of their time indoors. [31] The amount of time spent indoors depends upon on several factors including geographical region, job activities, and gender among other variables. Additionally, because home insulation is improving, this can result in greater retention of indoor air pollutants, such as NO2. [31] With respect to geographic region, the prevalence of asthma has ranged from 2 to 20% with no clear indication as to what's driving the difference. [31] This may be a result of the "hygiene hypothesis" or "western lifestyle" that captures the notions of homes that are well insulated and with fewer inhabitants. [31] Another study examined the relationship between nitrogen exposure in the home and respiratory symptoms and found a statistically significant odds ratio of 2.23 (95% CI: 1.06, 4.72) among those with a medical diagnosis of asthma and gas stove exposure. [32]

A major source of indoor exposure to NO2 is the use of gas stoves for cooking or heating in homes. According to the 2000 census, over half of US households use gas stoves [33] and indoor exposure levels of NO2 are, on average, at least three times higher in homes with gas stoves compared to electric stoves with the highest levels being in multifamily homes. Exposure to NO2 is especially harmful for children with asthma. Research has shown that children with asthma who live in homes with gas stoves have greater risk of respiratory symptoms such as wheezing, cough and chest tightness. [32] [34] Additionally, gas stove use was associated with reduced lung function in girls with asthma, although this association was not found in boys. [35] Using ventilation when operating gas stoves may reduce the risk of respiratory symptoms in children with asthma.

In a cohort study with inner-city minority African American Baltimore children to determine if there was a relationship between NO2 and asthma for children aged 2 to 6 years old, with an existing medical diagnosis of asthma, and one asthma related visit, families of lower socioeconomic status were more likely to have gas stoves in their homes. The study concluded that higher levels of NO2 within a home were linked to a greater level of respiratory symptoms among the study population. This further exemplifies that NO
2 toxicity is dangerous for children. [36]

Environmental effects

Interaction of NO2 and other NOx with water, oxygen and other chemicals in the atmosphere can form acid rain which harms sensitive ecosystems such as lakes and forests. [37] Elevated levels of NO
2 can also harm vegetation, decreasing growth, and reduce crop yields. [38]

See also

Related Research Articles

<span class="mw-page-title-main">Nitrogen</span> Chemical element, symbol N and atomic number 7

Nitrogen is a chemical element; it has symbol N and atomic number 7. Nitrogen is a nonmetal and the lightest member of group 15 of the periodic table, often called the pnictogens. It is a common element in the universe, estimated at seventh in total abundance in the Milky Way and the Solar System. At standard temperature and pressure, two atoms of the element bond to form N2, a colorless and odorless diatomic gas. N2 forms about 78% of Earth's atmosphere, making it the most abundant uncombined element in air. Because of the volatility of nitrogen compounds, nitrogen is relatively rare in the solid parts of the Earth.

<span class="mw-page-title-main">Nitric acid</span> Highly corrosive mineral acid

Nitric acid is the inorganic compound with the formula HNO3. It is a highly corrosive mineral acid. The compound is colorless, but samples tend to acquire a yellow cast over time due to decomposition into oxides of nitrogen. Most commercially available nitric acid has a concentration of 68% in water. When the solution contains more than 86% HNO3, it is referred to as fuming nitric acid. Depending on the amount of nitrogen dioxide present, fuming nitric acid is further characterized as red fuming nitric acid at concentrations above 86%, or white fuming nitric acid at concentrations above 95%.

<span class="mw-page-title-main">Nitronium ion</span> Polyatomic ion

The nitronium ion, [NO2]+, is a cation. It is an onium ion because its nitrogen atom has +1 charge, similar to ammonium ion [NH4]+. It is created by the removal of an electron from the paramagnetic nitrogen dioxide molecule NO2, or the protonation of nitric acid HNO3.

<span class="mw-page-title-main">Oxide</span> Chemical compound where oxygen atoms are combined with atoms of other elements

An oxide is a chemical compound containing at least one oxygen atom and one other element in its chemical formula. "Oxide" itself is the dianion of oxygen, an O2– ion with oxygen in the oxidation state of −2. Most of the Earth's crust consists of oxides. Even materials considered pure elements often develop an oxide coating. For example, aluminium foil develops a thin skin of Al2O3 that protects the foil from further oxidation.

<span class="mw-page-title-main">Ozone</span> Allotrope of oxygen (O₃) present in Earths atmosphere

Ozone is an inorganic molecule with the chemical formula O
3. It is a pale blue gas with a distinctively pungent smell. It is an allotrope of oxygen that is much less stable than the diatomic allotrope O
2, breaking down in the lower atmosphere to O
2 (dioxygen). Ozone is formed from dioxygen by the action of ultraviolet (UV) light and electrical discharges within the Earth's atmosphere. It is present in very low concentrations throughout the atmosphere, with its highest concentration high in the ozone layer of the stratosphere, which absorbs most of the Sun's ultraviolet (UV) radiation.

The Ostwald process is a chemical process used for making nitric acid (HNO3). Wilhelm Ostwald developed the process, and he patented it in 1902. The Ostwald process is a mainstay of the modern chemical industry, and it provides the main raw material for the most common type of fertilizer production. Historically and practically, the Ostwald process is closely associated with the Haber process, which provides the requisite raw material, ammonia (NH3).

<span class="mw-page-title-main">Oxidizing agent</span> Chemical compound used to oxidize another substance in a chemical reaction

An oxidizing agent is a substance in a redox chemical reaction that gains or "accepts"/"receives" an electron from a reducing agent. In other words, an oxidizer is any substance that oxidizes another substance. The oxidation state, which describes the degree of loss of electrons, of the oxidizer decreases while that of the reductant increases; this is expressed by saying that oxidizers "undergo reduction" and "are reduced" while reducers "undergo oxidation" and "are oxidized". Common oxidizing agents are oxygen, hydrogen peroxide, and the halogens.

<span class="mw-page-title-main">Dinitrogen tetroxide</span> Chemical compound

Dinitrogen tetroxide, commonly referred to as nitrogen tetroxide (NTO), and occasionally (usually among ex-USSR/Russia rocket engineers) as amyl, is the chemical compound N2O4. It is a useful reagent in chemical synthesis. It forms an equilibrium mixture with nitrogen dioxide. Its molar mass is 92.011 g/mol.

<span class="mw-page-title-main">Red fuming nitric acid</span> Chemical compound

Red fuming nitric acid (RFNA) is a storable oxidizer used as a rocket propellant. It consists of 84% nitric acid, 13% dinitrogen tetroxide and 1–2% water. The color of red fuming nitric acid is due to the dinitrogen tetroxide, which breaks down partially to form nitrogen dioxide. The nitrogen dioxide dissolves until the liquid is saturated, and produces toxic fumes with a suffocating odor. RFNA increases the flammability of combustible materials and is highly exothermic when reacting with water.

<span class="mw-page-title-main">Nitric oxide</span> Colorless gas with the formula NO

Nitric oxide is a colorless gas with the formula NO. It is one of the principal oxides of nitrogen. Nitric oxide is a free radical: it has an unpaired electron, which is sometimes denoted by a dot in its chemical formula. Nitric oxide is also a heteronuclear diatomic molecule, a class of molecules whose study spawned early modern theories of chemical bonding.

Nitrogen oxide may refer to a binary compound of oxygen and nitrogen, or a mixture of such compounds:

<span class="mw-page-title-main">Nitrous acid</span> Chemical compound

Nitrous acid is a weak and monoprotic acid known only in solution, in the gas phase, and in the form of nitrite salts. It was discovered by Carl Wilhelm Scheele, who called it "phlogisticated acid of niter". Nitrous acid is used to make diazonium salts from amines. The resulting diazonium salts are reagents in azo coupling reactions to give azo dyes.

<span class="mw-page-title-main">Dinitrogen pentoxide</span> Chemical compound

Dinitrogen pentoxide is the chemical compound with the formula N2O5. It is one of the binary nitrogen oxides, a family of compounds that only contain nitrogen and oxygen. It exists as colourless crystals that sublime slightly above room temperature, yielding a colorless gas.

The lead chamber process was an industrial method used to produce sulfuric acid in large quantities. It has been largely supplanted by the contact process.

In atmospheric chemistry, NOx is shorthand for nitric oxide and nitrogen dioxide, the nitrogen oxides that are most relevant for air pollution. These gases contribute to the formation of smog and acid rain, as well as affecting tropospheric ozone.

The chemical element nitrogen is one of the most abundant elements in the universe and can form many compounds. It can take several oxidation states; but the most common oxidation states are -3 and +3. Nitrogen can form nitride and nitrate ions. It also forms a part of nitric acid and nitrate salts. Nitrogen compounds also have an important role in organic chemistry, as nitrogen is part of proteins, amino acids and adenosine triphosphate.

<span class="mw-page-title-main">Birkeland–Eyde process</span>

The Birkeland–Eyde process was one of the competing industrial processes in the beginning of nitrogen-based fertilizer production. It is a multi-step nitrogen fixation reaction that uses electrical arcs to react atmospheric nitrogen (N2) with oxygen (O2), ultimately producing nitric acid (HNO3) with water. The resultant nitric acid was then used as a source of nitrate (NO3−) in the reaction which may take place in the presence of water or another proton acceptor.

<span class="mw-page-title-main">Reactive nitrogen species</span>

Reactive nitrogen species (RNS) are a family of antimicrobial molecules derived from nitric oxide (•NO) and superoxide (O2•−) produced via the enzymatic activity of inducible nitric oxide synthase 2 (NOS2) and NADPH oxidase respectively. NOS2 is expressed primarily in macrophages after induction by cytokines and microbial products, notably interferon-gamma (IFN-γ) and lipopolysaccharide (LPS).

<span class="mw-page-title-main">Nitrogen dioxide poisoning</span> Medical condition

Nitrogen dioxide poisoning is the illness resulting from the toxic effect of nitrogen dioxide. It usually occurs after the inhalation of the gas beyond the threshold limit value. Nitrogen dioxide is reddish-brown with a very harsh smell at high concentrations, at lower concentrations it is colorless but may still have a harsh odour. Nitrogen dioxide poisoning depends on the duration, frequency, and intensity of exposure.

<span class="mw-page-title-main">Transition metal nitrate complex</span> Compound of nitrate ligands

A transition metal nitrate complex is a coordination compound containing one or more nitrate ligands. Such complexes are common starting reagents for the preparation of other compounds.

References

  1. ↑ "nitrogen dioxide (CHEBI:33101)". Chemical Entities of Biological Interest (ChEBI). UK: European Bioinformatics Institute. 13 January 2008. Main. Archived from the original on 4 March 2016. Retrieved 4 October 2011.
  2. 1 2 3 4 Haynes, 4.79.
  3. ↑ Mendiara, S. N.; Sagedahl, A.; Perissinotti, L. J. (2001). "An electron paramagnetic resonance study of nitrogen dioxide dissolved in water, carbon tetrachloride and some organic compounds". Applied Magnetic Resonance. 20 (1–2): 275–287. doi:10.1007/BF03162326. S2CID   97875925.
  4. ↑ Haynes, 4.134.
  5. ↑ Haynes, 5.16.
  6. 1 2 "Nitrogen dioxide". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  7. 1 2 3 4 5 NIOSH Pocket Guide to Chemical Hazards. "Nitrogen dioxide". National Institute for Occupational Safety and Health (NIOSH).
  8. 1 2 PD-icon.svg This article incorporates public domain material from Nitrogen dioxide. United States Environmental Protection Agency. Feb 23, 2016.
  9. ↑ "Immediately Dangerous to Life or Health Concentrations (IDLH): Nitrogen dioxide". The National Institute for Occupational Safety and Health (NIOSH). May 1994. Retrieved October 20, 2023.
  10. 1 2 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 455-7. ISBN   978-0-08-037941-8.
  11. 1 2 3 Holleman, A. F.; Wiberg, E. (2001) Inorganic Chemistry. Academic Press: San Diego. ISBN   0-12-352651-5.
  12. ↑ physical chemistry
  13. ↑ Thiemann, Michael; Scheibler, Erich; Wiegand, Karl Wilhelm (2005). "Nitric Acid, Nitrous Acid, and Nitrogen Oxides". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a17_293. ISBN   978-3-527-30673-2.
  14. ↑ Finlayson-Pitts, B. J.; Wingen, L. M.; Sumner, A. L.; Syomin, D.; Ramazan, K. A. (2002-12-16). "The heterogeneous hydrolysis of NO2 in laboratory systems and in outdoor and indoor atmospheres: An integrated mechanism" (PDF). Physical Chemistry Chemical Physics. 5 (2): 223–242. doi:10.1039/B208564J.
  15. ↑ WHO Air Quality Guidelines – Second Edition. Chapter 7.1 Nitrogen Dioxide.
  16. ↑ Subcommittee on Emergency and Continuous Exposure Guidance Levels for Selected Submarine Contaminants; Committee on Toxicology; Board on Environmental Studies and Toxicology; Division on Earth and Life Studies; National Research Council. Chapter 12: Nitrogen Dioxide in Emergency and Continuous Exposure Guidance Levels for Selected Submarine Contaminants. National Academies Press, 2007. ISBN   978-0-309-09225-8
  17. ↑ "Mechanism Overview, June 2012" (PDF). noxilizer.com. Noxilizer, Inc. Archived from the original (PDF) on 12 April 2016. Retrieved 2 July 2013.
  18. ↑ Cotton, Simon (21 March 2013) Nitrogen dioxide. RSC Chemistry World.
  19. ↑ "Air quality guidelines – global update 2005". WHO. Archived from the original on March 9, 2014. Retrieved 2016-10-19.
  20. ↑ US Dept. of Health and Human Services, Public Health Service, Agency for Toxic Substances and Disease Registry, Division of Toxicology. April 2002 ATSDR Nitrous Oxides.
  21. ↑ "The Impact of Unvented Gas Heating Appliances on Indoor Nitrogen Dioxide Levels in 'TIGHT' Homes" (PDF). ahrinet.org. 2013-03-21. Archived from the original (PDF) on 2020-08-05. Retrieved 2018-09-25.
  22. ↑ Chan-Yeung, M.; Ashley, M. J.; Grzybowski, S. (1978). "Grain dust and the lungs". Canadian Medical Association Journal. 118 (10): 1271–4. PMC   1818652 . PMID   348288.
  23. ↑ Gurney, J. W.; Unger, J. M.; Dorby, C. A.; Mitby, J. K.; von Essen, S. G. (1991). "Agricultural disorders of the lung". Radiographics. 11 (4): 625–34. doi: 10.1148/radiographics.11.4.1887117 . PMID   1887117.
  24. 1 2 U.S. EPA. Integrated Science Assessment for Oxides of Nitrogen – Health Criteria (2016 Final Report). U.S. Environmental Protection Agency, Washington, DC, EPA/600/R-15/068, 2016. Federal Register Notice Jan 28, 2016 Free download available at Report page at EPA website.
  25. ↑ Toxnet Nitrogen dioxide: Human Health Effects Page accessed March 28, 2016.
  26. ↑ CDC NIOSH International Chemical Safety Cards (ICSC): Nitrogen Dioxide Page last reviewed: July 22, 2015; Page last updated: July 1, 2014.
  27. ↑ Agency for Toxic Substances and Disease Registry via the CDC Medical Management Guidelines for Nitrogen Oxides Page last reviewed: October 21, 2014; Page last updated: October 21, 2014
  28. ↑ University of Kansas Hospital, Poison Control Center Poison Facts: Medium Chemicals: Nitrogen Dioxide Archived 2016-04-11 at the Wayback Machine page accessed March 28, 2016
  29. ↑ "40 C.F.R.: Appendix A to Part 355—The List of Extremely Hazardous Substances and Their Threshold Planning Quantities" (PDF) (July 1, 2008 ed.). Government Printing Office. Archived from the original (PDF) on February 25, 2012. Retrieved October 29, 2011.
  30. ↑ Int Panis, L (2017). "Short-term air pollution exposure decreases lung function: a repeated measures study in healthy adults". Environmental Health. 16 (1): 60. doi: 10.1186/s12940-017-0271-z . PMC   5471732 . PMID   28615020.
  31. 1 2 3 4 Heinrich, Joachim (2011-01-01). "Influence of indoor factors in dwellings on the development of childhood asthma". International Journal of Hygiene and Environmental Health. 214 (1): 1–25. doi:10.1016/j.ijheh.2010.08.009. PMID   20851050.
  32. 1 2 Garrett, Maria H.; Hooper, Martin A.; Hooper, Beverley M.; Abramson, Michael J. (1998-09-01). "Respiratory Symptoms in Children and Indoor Exposure to Nitrogen Dioxide and Gas Stoves" (PDF). American Journal of Respiratory and Critical Care Medicine. 158 (3): 891–895. doi:10.1164/ajrccm.158.3.9701084. PMID   9731022.
  33. ↑ "Historical Census of Housing Tables -House Heating Fuel". www.census.gov. Retrieved 2016-10-19.
  34. ↑ PD-icon.svg This article incorporates public domain material from Nitrogen Dioxide Basic Information. United States Environmental Protection Agency . Retrieved February 23, 2016.
  35. ↑ Chapman, Robert S.; Hadden, Wilbur C.; Perlin, Susan A. (2003-07-15). "Influences of asthma and household environment on lung function in children and adolescents: the third national health and nutrition examination survey". American Journal of Epidemiology. 158 (2): 175–189. doi: 10.1093/aje/kwg129 . PMID   12851231.
  36. ↑ Hansel, Nadia N.; Breysse, Patrick N.; McCormack, Meredith C.; Matsui, Elizabeth C.; Curtin-Brosnan, Jean; Williams, D'Ann L.; Moore, Jennifer L.; Cuhran, Jennifer L.; Diette, Gregory B. (2016-10-19). "A Longitudinal Study of Indoor Nitrogen Dioxide Levels and Respiratory Symptoms in Inner-City Children with Asthma". Environmental Health Perspectives. 116 (10): 1428–1432. doi:10.1289/ehp.11349. PMC   2569107 . PMID   18941590.
  37. ↑ US EPA, OAR (2016-07-06). "Basic Information about NO2". US EPA. Retrieved 2020-07-03.
  38. ↑ "Nitrogen oxides". Queensland Government. Retrieved 2020-07-03.

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